Free Printable Honors Chem Ch 14

1.

What is the pH of a 0.72 M HBr solution?

(type the answer like this: 0.???

With a zero to the left of the decimal and 3 digits after the decimal)

(a)

2.

What is the pOH of a solution that has a pH of 3.98?

a)

10.02

b)

1.05 x 10^-4

c)

9.55 x 10^-11

d)

3.98

3.

Label the following as acid or base, or conjugate acid or conjugate base.

HCl + NH₃ --> Cl^- + NH₄⁺

a)

HCl

1.

acid

b)

NH₃

2.

base

c)

Cl^-

3.

conjugate base

d)

NH₄⁺

4.

conjugate acid

4.

Label the following as either acid or base or conjugate acid or conjugate base:

HClO + CH₃NH₂ --> ClO^- + CH₃NH₃⁺

a)

HClO

1.

acid

b)

CH₃NH₂

2.

base

c)

ClO^-

3.

conjugate base

d)

CH₃NH₃⁺

4.

conjugate acid

5.

What is the name of this compound: HNO₃

a)

nitric acid

b)

nitrous acid

c)

hydronitric acid

d)

hydronitrous acid

6.

What is the name of this compound: H₂SO₃

a)

sulfuric acid

b)

sulfurous acid

c)

hydrosulfurous acid

d)

hydrosulfate acid

7.

What is the name of this compound: HBr

a)

bromic acid

b)

broumous acid

c)

hydrobromic acid

d)

hydrobromous acid

8.

What is the name of this compound: KOH

a)

potassium hydroxide

b)

potassium oxygen hydride

c)

hydroxide potassium

d)

potassium monohydroxide

9.

What is the name of this compound: Ca(OH)₂

a)

calcium dihydroxide

b)

calcium bihydroxide

c)

calcium hydroxide

d)

hydroxide dicalcium

10.

What is the [OH-] in a solution that has a [H3O+] of 1.35 x 10^-4

a)

1.35 x 10¹⁰

b)

13.999865

c)

7.41 x 10^-19

d)

7.41 x 10^-11

11.

If the [OH^-] in a hydrochloric acid solution is 8.91 x 10^-12, what is the hydronium ion concentration?

a)

1.12 x 10^-3

b)

1.12 x 10^-27

c)

8.91 x 10^-26

d)

891

12.

What is the acid dissociation reaction for HF dissolving in water?

a)

HF + H2O $\leftrightarrow$ F + H₃O

b)

HF + H2O $\leftrightarrow$ F^- + H₃O⁺

c)

HF + H2O $\leftrightarrow$ H_²F⁺ + OH^-

13.

If 150.0 g of hydroiodic acid, HI, dissolved in 1.25 L of solution, what is the [H3O+] and [OH-]? (choose two)

a)

[H₃O⁺] = 0.938M

b)

[OH-] = 1.07x10^-14M

c)

[OH-] = 0.938M

d)

[H₃O⁺] = 1.07x10^-14M

14.

What is the [OH-] in a solution where 0.75 mols of Ca(OH)₂ dissolves in water to make 1.45 L of solution?

a)

0.517 M

b)

1.03 M

c)

0.259 M

d)

0.75 M

15.

What is the pH of a solution that has a [H3O+] of 2.18 x 10^-5?

a)

1.0 x 10^-14

b)

4.59 x 10^-10

c)

4.66

d)

9.34

16.

What is the pH of a solution where the [OH-] is 1.38 x 10^-3?

a)

2.86

b)

7.25 x 10^-12

c)

11.14

d)

3.18

17.

In a solution, the [H3O+] is 3.17 x 10^-4and the [OH-] is 3.15 x 10^-11. Is this solution acidic or basic and why?

a)

basic b/c [H3O+] > [OH-]

b)

acidic b/c [H3O+] > [OH-]

c)

basic b/c [H3O+] < [OH-]

d)

acidic b/c [H3O+] < [OH-]

18.

If the K_a of a 0.25M weak acid is 3.5 x 10^-6, what is the pH?

a)

6.06

b)

3.03

c)

7.94

d)

10.97

19.

What is the pH of a 0.35M weak base with a K_b of 2.4 x 10^-7?

a)

7.08

b)

6.92

c)

10.46

d)

3.54

20.

Write the Ka expression for the following reaction:

HCN(aq) + H₂O(l) $\leftrightarrow$ CN^-(aq) + H₃O⁺(aq)

a)

Ka = [HCN][H₂O] / [CN^-][H₃O⁺]

b)

Ka = [HCN] /

[CN^-][H₃O⁺]

c)

Ka = [CN^-][H₃O⁺] / [HCN]

d)

Ka = [CN^-][H₃O⁺] / [HCN][H₂O]

21.

Which one is the strongest acid?

a)

HCN (Ka = 4.9 x 10^-10)

b)

HClO (Ka = 3.0 x 10^-8)

c)

HNO₂ (Ka = 4.5 x 10^-4)

d)

HF (Ka = 6.8 x 10^-4)

22.

What is the conjugate acid of NH₃?

a)

NH₃

b)

NH₄⁺

c)

NH₂^-

d)

H₂O

23.

What is the conjugate base of HCN?

a)

HCN

b)

H₂CN⁺

c)

CN^-

d)

H₂O

24.

Which two are amphiprotic? (choose two)

a)

H2O

b)

NaOH

c)

HCl

d)

HSO₄^-

25.

What is the [OH^-] in an HCl solution that has a pH of 2.31?

a)

1 x 10^-14

b)

4.90 x 10^-3

c)

2.04 x 10^-12

d)

11.69

26.

Calculate the pH of the resulting solution when 35.0 mL of 0.15M HCl is mixed with 45.0 mL of 0.13M NaOH.

a)

2.12

b)

11.88

c)

0.0006

d)

1.70

e)

3.87

27.

Calculate the pH of the resulting solution when 50.0 mL of 0.25M HCl is mixed with 75.0 mL of 0.24M NaOH.

a)

12.64

b)

1.36

c)

0.044

d)

0.0055

e)

12.02

28.

Complete the acid dissociation reaction for hypobromous acid, HBrO:

HBrO + (a) --> (b) + H3O+

Choose from the below words

BrO-

H2O

OH-

H2BrO+

BrO

H3O+

HBrO

29.

Complete the acid dissociation reaction for chromic acid, H₂CrO₄:

H₂CrO₄ + (a) --> (b) + H3O+

Choose from the below words

HCrO4(-)

H2O

OH-

H3CrO4(+)

CrO4

H3O+

HCrO

30.

Complete the acid dissociation reaction for hypobromous acid, HBrO:

(a) + H2O --> (b) + H3O+

Choose from the below words

BrO-

OH-

H2BrO+

BrO

H3O+

HBrO

H2O

31.

Complete the acid dissociation reaction for chromic acid, H₂CrO₄:

(a) + H2O --> (b) + H3O+

Choose from the below words

HCrO4(-)

OH-

H2CrO4(+)

CrO

H3O+

H2CrO4

H2O

32.

Complete the acid dissociation reaction for hypobromous acid, HBrO:

(a) + H2O --> BrO^- + (b)

Choose from the below words

OH-

H2BrO+

BrO

H3O+

HBrO

H2O

BrO-

33.

Complete the acid dissociation reaction for hypobromous acid, H₂CrO₄:

(a) + H2O --> HCrO₄^- + (b)

Choose from the below words

OH-

H2CrO4(+)

CrO4

H3O+

H2CrO4

H2O

CrO4(2-)

34.

Write the acid dissociation expression, Ka, for this reaction:

H₃BO₃(aq) + H₂O(l) ↔ H₂BO₃^-(aq) + H₃O⁺(aq)

a)

Ka = $\frac{\left[H_2BO_3^-\right]\left[H_3O^+\right]}{\left[H_3BO_3\right]}$

b)

Ka = $\frac{\left[H_2BO_3^-\right]\left[H_3O^+\right]}{\left[H_3BO_3\right]\left[H_2O\right]}$

c)

Ka = $\frac{\left[H_3BO_3\right]}{\left[H_2BO_3^-\right]\left[H_3O^+\right]}$

d)

Ka = $\frac{\left[H_3BO_3\right]\left[H_2O\right]}{\left[H_2BO_3^-\right]\left[H_3O^+\right]}$

e)

[H₃BO₃][H₂O] = [B₂BO₃^-][H₃O⁺]

35.

Write the acid dissociation expression, Ka, for this reaction:

HClO₂(aq) + H₂O(l) ↔ ClO₂^-(aq) + H₃O⁺(aq)

a)

Ka = $\frac{\left[ClO_2^-\right]\left[H_3O^+\right]}{\left[HClO_2\right]}$

b)

Ka = $\frac{\left[ClO_2^-\right]\left[H_3O^+\right]}{\left[HClO_2\right]\left[H_2O\right]}$

c)

Ka = $\frac{\left[HClO_2\right]}{\left[ClO_2^-\right]\left[H_3O^+\right]}$

d)

Ka = $\frac{\left[HClO_2\right]\left[H_2O\right]}{\left[ClO_2^-\right]\left[H_3O^+\right]}$

e)

[HClO₂][H₂O] = [ClO₂^-][H₃O⁺]

36.

Write the acid dissociation expression, Ka, for this reaction:

HCl(aq) + H₂O(l) → Cl^-(aq) + H₃O⁺(aq)

a)

Ka = $\frac{\left[Cl^-\right]\left[H_3O^+\right]}{\left[HCl\right]}$

b)

Ka = $\frac{\left[Cl^-\right]\left[H_3O^+\right]}{\left[HCl\right]\left[H_2O\right]}$

c)

Ka = $\frac{\left[HCl\right]}{\left[Cl^-\right]\left[H_3O^+\right]}$

d)

Ka = $\frac{\left[HCl\right]\left[H_2O\right]}{\left[Cl^-\right]\left[H_3O^+\right]}$

e)

[HCl][H₂O] = [Cl^-][H₃O⁺]

37.

A 20.0 mL sample of HCl with unknown concentration was titrated with 16.57 mL of 0.35M NaOH.

What is the concentration of the HCl?

a)

0.290 M

b)

2.90 M

c)

0.422 M

d)

4.22 M

e)

0.159 M

38.

A 15.00 mL sample of NaOH with unknown concentration was titrated with 21.28 mL of 0.16 M HCl.

What is the concentration of the NaOH?

a)

0.227 M

b)

2.27 M

c)

0.113 M

d)

1.13 M

e)

0.0938 M

39.

A student needs to make 500.0 mL of a 1.25 M NaOH solution. How many grams of solid NaOH should they weigh out to pour into a 500.0 mL volumetric flask and dissolve with water?

The molar mass of NaOH = 40.00 g/mol

a)

25.0 grams

b)

1.25 grams

c)

40.00 grams

d)

2500 grams

e)

35.00 grams

40.

What is a binary acid?

H⁺ plus (a) more element(s).

How is a binary acid named?

(b) the (c) prefix and change the ending to (d)

Choose from the below words

one

Use

-ic

hydro-

Do not use

-ous

-ate

-ite

two

41.

What is an oxyacid?

H⁺ plus a (a) .

How is an oxyacid named?

(b) the hydro- prefix and the ending changes:

from -ate to (c)

or

from (d) to (e)

Choose from the below words

Use

Do not use

-ous

-ite

two

polyatomic ion

-ic

monatomic ion

hydrocarbon

-ide

42.

Name the following binary acids:

HCl (a)

HBr (b)

HF (c)

Choose from the below words

hydrochloric acid

chloric acid

hydrobromic acid

bromic acid

Hydrofluoric acid

fluoric acid

43.

Name the following oxyacids acids:

~~hydro~~ + polyatomic + ic or ous + acid

HClO (a)

HClO₂ (b)

HClO₃ (c)

HClO₄ (d)

Choose from the below words

hydrochloric acid

hypochlorous acid

chlorous acid

chloric acid

perchloric acid

chlorite acid

chlorate acid

hypochlorate acid

perchlorous acid

44.

What is the conjugate base of HCl?

a)

Cl^-

b)

Cl

c)

C

d)

H₂Cl

45.

What is the conjugate base of H₂SO₄?

a)

HSO₄^-

b)

SO₄

c)

H₃SO₄

d)

HSO

46.

What is the conjugate acid of H₂O?

a)

OH^-

b)

H₃O⁺

c)

HO

d)

HO₂

47.

What is the conjugate acid of NH₃?

a)

NH₄⁺

b)

NH4

c)

NH₂

d)

N

48.

Organize these molecules into the right categories

Categorize the following

HCl

NaOH

H2O

NaCl

Acids

Bases

Amphiprotic

Neither

49.

Complete this reaction in this order:

acid + base → c. base + c. acid

HNO₃ + OH^- → (a) + (b)

Choose from the below words

NO3-

H2O

H3O+

NO-

50.

Complete this reaction in this order:

base + acid → c. acid + c. base

NH₃ + H₃O⁺ → (a) + (b)

Choose from the below words

NH4+

H2O

H3O+

NH4

NH2-

OH-

51.

The equilibrium expression for water, Kw, is: K_w = [H₃O⁺][OH^-]

and K_w = 1.0 x 10^-14

Rearrange the equation two times:

[H₃O⁺] = (a) / (b)

[OH^-] = (c) / (d)

Choose from the below words

1.0 x 10^-14

[OH-]

[H3O+]

H2O

[H3O]

[OH]

52.

A solution has a hydroxide, OH^-, concentration of [OH^-] = 1.5 x 10^-4. What is the [H₃O⁺] concentration?

Show work:

1.0 x 10^-14 / (a) = (b)

Choose from the below words

1.5 x 10^-4

6.7 x 10^-11

6.7 x 10^-19

53.

45.0 grams of KOH is dissolved in 1.50 L of water. To calculate the molarity of OH- in the solution, follow this:

45.0 g KOH / (56.1 g/mol) = 0.8021 mols

0.8021 mols / 1.50 L = 0.5348M OH^-

Calculate the [H3O+] in the solution.

a)

0.535 M

b)

1.87 x 10^-14

c)

56.1 g/mol

d)

5.35 x 10¹³

54.

45.0 grams of KOH is dissolved in 1.50 L of water. Calculate the [OH^-] in the solution.

a)

0.535 M

b)

1.87 x 10^-14M

c)

56.1 g/mol

d)

5.35 x 10¹³M

e)

0.802 mol

55.

An acid and a base react together and neutralize each other. They always produce:

a)

CO2 and water

b)

a salt and water

c)

CO2 and a salt

d)

CO2 and O2

e)

water and O2

56.

What are the two products of HF and LiOH reacting together?

a)

H2O

b)

LiF

c)

H3O⁺

d)

OH^-

e)

Li₂F

57.

When 440 mL of 3.1 M HClO₄ is mixed with 220 mL of 4.1 M LiOH, what is the pH of the resulting solution?

a)

pH = 0.15

b)

pH = 0.70

c)

pH = 0.462

d)

pH = 0.902

58.

Before a titration experiment is begun, NaOH is filled in the buret until it's a little below the zero. The value is recorded as:

a)

1.40

b)

2.60

c)

1.50

d)

2.70

e)

1.10

59.

At the end of the titration, the value in the buret is recorded again. What is the value recorded as?

a)

20.60

b)

21.40

c)

26.00

d)

24.00

60.

The image shows the buret before and after a titration. What is the value of the titrant used in this titration?

Show calculation and record correct sig figs for all values.

a)

27.30 - 0.45 = 26.85 mL

b)

28.70 - 1.55 = 27.15 mL

c)

27.3 - 0.5 = 26.8 mL

d)

28.7 - 1.6 = 27.1 mL

e)

28.7 mL (no calculation necessary)

61.

What is the initial value recorded for this titration? (a)

What is the final value recorded for this titration? (b)

What is the value of the titrant used? (c)

Choose from the below words

1.25 mL

2.75 mL

27.75 mL

28.25 mL

26.50 mL

25.50 mL

62.

15.0 mL of HI is titrated with 3.0 M of LiOH. Once 19.6 mL of the 3.0M LiOH was added, the solution turned light pink and the titration was complete. What is the Molarity of the HI?

Hint: Use M_aV_a = M_bV_b to solve for M_a

a)

3.92

b)

98

c)

882

d)

0.435

e)

2.296

63.

A 25.0 mL solution of HF was titrated with 0.10M solution of NaOH. Before the titration began, the buret read 1.50 mL and after the titration was complete the buret read 24.70 mL. What is the volume of NaOH used in this titration?

a)

23.20 mL

b)

24.70 mL

c)

1.50 mL

d)

26.20 mL

e)

25.00 mL

64.

A 22.0 mL solution of HF was titrated with 0.10M solution of NaOH. Before the titration began, the buret read 1.50 mL and after the titration was complete the buret read 24.7 mL.

The volume of NaOH used was 24.70 - 1.50 mL = 23.20 mL

What is the concentration of HF?

HF + NaOH → NaF + H2O

M_aV_a = M_bV_b

a)

0.105 M

b)

51.0 M

c)

0.0948 M

d)

1.96x10^-4 M

e)

5104 M

Honors Chem Ch 14

Total questions: 64

Worksheet time: 3hrs 12mins

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